In the reaction, F₂ + 2NaOH $\to$2NaF + OF₂ + H₂O, which undergoes oxidation?

$\stackrel{0}{{\mathrm{F}}_2}+2\stackrel{+1}{\mathrm{Na}}\stackrel{-2}{\mathrm{O}}\stackrel{+1}{\mathrm{H}}\to 2\stackrel{+1}{\mathrm{Na}}\stackrel{-1}{\mathrm{F}}+\stackrel{+2}{\mathrm{O}}{\stackrel{-1}{\mathrm{F}}}_2+{\stackrel{+1}{\mathrm{H}}}_2\stackrel{-2}{\mathrm{O}}$

F₂ undergoes reduction(0 to -1)
F₂ is the Oxidising agent
NaOH undergoes Oxidation (Ox. state of Oxygen changes from -2 to +2)
NaOH is the reducing agent
Elements undergoing Oxidation is Oxygen